i dont think im on the right track for question 2 1. The specific heat of aluminum is 0.900 J/°C g.Problems:The specific heat of aluminum is 0.900 J/°C g.d. How much heat energy is needed to raise the temperature of a 8.50 x 102 g block of aluminumfrom 22.8 °C to 94.6 °C?b. Calculate the molar heat capacity of aluminum.A 45.0 g block of metal at 99.5 °C was dropped into 150.0 g of water at 24.00 °C. The temperatureof the mixture rose to 26.40 °C. The specific heat of water is 4.184 J/g°C. Determine the specificheat of the metal.A 200 g piece of lead (0.0305 cal/g K) is heated to 90 °C and dropped into 500 g of water, initiallyat 20 °C. Neglecting the heat capacity of the container, find the final temperature of the lead andwater. (H2O: 1.00 cal/g-K)4.A 30 g piece of ice, falling off the space shuttle through the Earth's atmosphere, reached a consterminal velocity of 8 m/s. Assuming no heat is lost to the surroundings, how far will it have toin order for all the ice to be melted before it hits the ground? The latent heat of fusion for ice i80 cal/g.[Ans: 34 km]5.When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat fromof air at normal pressure is 1.015 J/g.°C. What is the change in air temperature, assumingof the air in the room, in g/crof steam is used to heat a room containing 6.44 x 104 g of air (20 ft x 12 ft x 8 ft). The specit2.3. Cs.Cうこて Mm- 4s.0a Tiz 99.5℃MwE150.0a Ti=Z4.00Csこ 4.184TE =26.40°C-145.0S((s)c26. )Cs)(26.4-9a.51-99.5)-158-004.184Y26.4-て4.00)cs1S06ペ.ム.184 2.445.0g-(-73.1)

Given: Mass of metal = 45.0 g. Initial temperature of metal = 99.5 oC Mass of water = 150.0 g…

A 45.0 g block of metal at 99.5 °C was dropped into 150.0 g of water at 24.00 °C. The temperature of the mixture rose to 26.40 °C. The specific heat of water is 4.184 J/g°C. Determine the specific heat of the metal. tor initially

A 45.0 g block of metal at 99.5 °C was dropped into 150.0 g of water at 24.00 °C. The temperature of the mixture rose to 26.40 °C. The specific heat of water is 4.184 J/g°C. Determine the specific heat of the metal. tor initially

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For questions #14-16, you should do your work on a separate piece of paper and then upload it. You should use the GUESS Method of solving for each problem. Also, you have a choice. You can complete both #14 & #15 which are single step question or do the extension problem which is a 2 step problem instead of 14 & 15. You must complete #16. Equations Q = mcAT Q = ±mLf Q = ±mLv Values for Water Clice) = 2.06 J/g°C C(water) = 4.186 J/g°C C(steam) = 1.87 J/g°C Lf (water) = 333 J/g Lv (water) = 2,260 J/g %3D G- S- U- E- S- #14. Calculate the energy required to heat 12.5 g of water from a temperature of 42.2°C to 52.3°C. #15. How much thermal energy is needed in order to turn 15.7 grams of water into ice? Extension: We start with 23.2 grams of ice at 0°C and add heat to the ice. The ice completely melts and then is heated until it reaches 45.3°C. How much energy is added in total? #16. 12.0 g of a metal absorbs 317 J when it is heated from 38.2°C to 82.7°C. What is the specific heat of the…
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